Exercise: The temperature dependence of the rate constant for the gas-phase reactionare as follows:NO(g) + O3(g)a. 1.40E+14b.C.1.60E+121.55E+14d. 1.55E+12Temperature (K)195230260298369Determine the value of frequency factor (A) for this reactionLn(k)=-Ea 1()+ LnARTe. 1.40E+12NO2(g)k1.08 10⁹2.95 × 10⁰5.42 × 10⁹12 × 10⁹35.5 × 10⁹+ O2(g)1/T (K™) Ln(k) Exercise: The temperature dependence of the rate constant for the gas-phase reactionare as follows:NO(g) + O3(g)a. 1.40E+14b.C.1.60E+121.55E+14d. 1.55E+12Temperature (K)195230260298369Determine the value of frequency factor (A) for this reactionLn(k)=-Ea 1()+ LnARTe. 1.40E+12NO2(g)k1.08 10⁹2.95 × 10⁰5.42 × 10⁹12 × 10⁹35.5 × 10⁹+ O2(g)1/T (K™) Ln(k)

for the given reaction the required data to plot the ln of rate vs. 1/T plot is given. It…

Exercise The temperature dependence of the rate constant for the gas-phase reaction are as follows: NO(g) + O3(g) NO2(g) + O2(g) a. 1.40E+14 b. C. 1.60E+12 Determine the value of frequency factor (A) for this reaction Ea 1 Ln(k)=- ()+ LnA RT 1.55E+14 Temperature (K) 195 230 260 298 369 d. 1.55E+12 e. 1.40E+12 k 1.08 x 10° 2.95 × 10⁹ 5.42 × 10⁹ 12 × 10⁹ 35.5 × 10⁹ 1/T (K¹) Ln(k) -

Exercise The temperature dependence of the rate constant for the gas-phase reaction are as follows: NO(g) + O3(g) NO2(g) + O2(g) a. 1.40E+14 b. C. 1.60E+12 Determine the value of frequency factor (A) for this reaction Ea 1 Ln(k)=- ()+ LnA RT 1.55E+14 Temperature (K) 195 230 260 298 369 d. 1.55E+12 e. 1.40E+12 k 1.08 x 10° 2.95 × 10⁹ 5.42 × 10⁹ 12 × 10⁹ 35.5 × 10⁹ 1/T (K¹) Ln(k) -

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.33PAE: The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution....

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The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
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(ii) At elevated temperatures, nitrogen dioxide decomposes to nitric oxide and molecular oxygen: 2NO2(g) – → 2NO(g) + O2(g) The change in concentration of NO2 with time at 300 °C is given below: t (s) 100 200 300 400 500 [NO2]/103 (mol dm-3) 8.0 5.6 4.3 3.5 2.9 2.5 By appropriate plotting of the data and use of this graph: (a) verify that this reaction is second order with respect to NO2; (b) determine the rate constant for this reaction.
The reaction 5 Br- (aq) + BrO3 (aq) + 6H+ (aq) ЗBr2 (1) + ЗН20 (1) is expected to obey the mechanism BrO3 (aq) + H* (aq) HBRO3 (ag) + H+ - HBRO3 (aq) - H2BRO3+ (aq) Fast Fast (aд) + H2BrO3™ (aq) + Br (aq) (Br-BrO2) (aq) + H2O (I) Slow (Br-BrO2) (aq) + 4H+ (aq) + 4Br" (aq) 3Br2 (1) + 3H20 (I) Fast Write the rate law.
For the gas phase decomposition of difluoroperoxide,F2O2F2 + O2the rate constant has been determined at several temperatures. When ln k in s-1 is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -8.71×103 K and a y-intercept of 29.4. The activation energy for the gas phase decomposition of difluoroperoxide is ______kJ/mol.
For the gas phase decomposition of dinitrogen pentoxide, N₂Os 2 NO₂+1/20₂ the rate constant has been determined at several temperatures. When Ink in s¹ is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -1.24 x 10 K and a y-intercept of 31.3. The activation energy for the gas phase decomposition of dinitrogen pentoxide is Submit Answer Retry Entire Group 1 more proun attempt remaining kJ/mol.
2. Consider the kinetic data of the reaction of P + 2 Q + 2+ - PQ, + Z*and answer the succeeding questions: Experiment P (M) Q (M) Temp ("C) Initial Rate, M/s 1 0.01150 0.01200 0.00000 25 4.80 x 10-4 2 0.02300 0.01200 0.00000 25 1.92 x 10-3 3 0.01150 0.02400 0.00000 25 9.60 x 10-4 4 0.04600 0.01200 0.00000 25 7.68 x 10-3 5 0.01150 0.04800 0.00000 25 1.92 x 10-3 6 0.01150 0.01200 0.00000 10 5.10 x 10-5 0.01150 0.01200 0.00000 40 4.55 x 10-3 0.01150 0.01200 0.00500 10 4.98 x 10-5 0.01150 0.01200 0.01050 25 4.82 x 104 10 0.01150 0.01200 0.02100 40 4.44 x 10-3 A. Determine the rate order with respect to P. Determine the rate order with respect to Q. C. Determine the rate law of the reaction. What is the average rate constant? Indicate the appropriate units. E. What is the energy of activation and frequency factor of the reaction without the additive ion? Include the equation of the best fit line of the Arrhenius equation and RSQ Note: Use the calculated rate constant in set up 1 for 25°C…
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The activation energy for the reaction NO2 (g) + CO(g) → NO(g) + CO2 (g) is E₁ = 350 kJ/mol and the change in enthalpy for the reaction is AH =-350 kJ/mol. What is the activation energy for the reverse reaction? Express your answer with the appropriate units. ► View Available Hint(s) 00 750 Submit μÅ kJ mol Previous Answers ? X Incorrect; Try Again; 4 attempts remaining
4) Use the data below to determine the rate law and the value of k for the following reaction CHC13 (g) + Cl2 (9) → CC14 (g) + HCl (g) [CHCI3] (M) [Cl2] (M) Initial Rate 0.0035 Experiment 1 0.010 0.010 2 0.020 0.010 0.0069 3 0.020 0.020 0.0098 4 0.040 0.040 0.0270
Experiment Temperature (K) [A], (M) Initial Rate (M/s) 1 298 1.00x10-3 7.76x10-9 2 323 1.00x10-3 1.17x10-7 347 1.00x10-3 1.10x10-6 4 369 1.00x10-3 6.61×10-6 The plot of the natural log of the rate constant vs. the reciprocal of the absolute temperature is which of the following? Linear Arrhenius Plot Linear Arrhenius Plot 400 0.008 300 0.006 y = 8183x + 318.231 200 0.004 y = 8.62E-5x - 0.0268 100 0.002 0.000 0.000 0.005 0.010 100 200 300 400 1/T 1/T Linear Arrhenius Plot 0.004 Linear Arrhenius Plot 0.000 -2.000 0.003 -4.000 y = -9.57E-5x + 0.00223 0.002 -6.000 -8.000 y = -10450x +23.301 0.001 F-10.000 -12.000 0.000 -14.000 -15.000 -10.000 -5.000 0.000 0.000 0.002 0.004 1/T 1/T Using the correct plot, determine the activation energy (in kJ/mol) and frequency factor (with appropriate units) for the reaction. activation energy, Ea 4.0 kJ/mol frequency factor, A 4.0 s-1 In k In k Ink In k